Balance the chemical equation given below, and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25 °C. The density of nitrogen monoxide at 25 °C is 1.23 g L^-1. ________ NH₃(g) + ________ O₂(g) → ________ NO(g) + ________ H₂O(l)

Question

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The balanced equation is 4 NH₃ + 5 O₂ → 4 NO + 6 H₂O. Moles of NH₃ = 8.00 g / 17.03 g/mol = 0.47 mol. Moles of O₂ = 12.0 g / 32.00 g/mol = 0.375 mol. O₂ is the limiting reactant. From the balanced equation, 5 moles of O₂ produce 4 moles of NO. Thus, 0.375 moles of O₂ produce (4/5) * 0.375 = 0.30 moles of NO. Mass of NO = 0.30 mol * 30.01 g/mol = 9.00 g. Volume of NO = 9.00 g / 1.23 g/L = 7.32 L.

Balance the Chemical Equation Given Below, and Calculate the Volume